N₂ (14) :
\( \sigma 1 s^{2}, \sigma^{*} 1 s^{2}, \sigma 2 s^{2}, \sigma^{*} 2 s^{2}, \pi 2 p_{x}^{2}=\pi 2 p_{y}^{2}, \sigma 2 p_{z}^{2} \)
\(\text { B.O. }=\frac{1}{2}(10-4)=\frac{6}{2}=3 \)
N₂ is diamagnetic because it does not have unpaired electron.

(i) sp²
(ii) Sp²,
(iii) sp,
(iv) sp, Sp²,
(v) Sp², Sp²

Electronic configuration of Be = 1s² 2s²
M.O. configuration of Be₂ = \((\sigma 1 s)^{2}\left(\sigma^{*} 1 s\right)^{2}(\sigma 2 s)^{2}\)\( \left(\sigma^{*} 2 s\right)^{2} \)
\(\text { Bond order of } \mathrm{Be}_{2}=\frac{1}{2}(4-4)=0 \)
Since bond order is zero it does not exist.

In H₂O, oxygen atom is sp³ hybridised with two lone pairs. The four sp³ hybridised orbitals acquire a tetrahedral geometry with two corners occupied by hydrogen atoms while other two by the lone pairs.
The bond angle is reduced to 104.5^o due to greater repulsive forces between lp - lp and the molecule thus acquires a V-shape or bent structure (angular structure).

In CO₂ molecule, carbon atom is sp-hybridised. The two sp hybrid are oriented in opposite direction forming an angle of 180^o \(O\overset { \pi }{ = } C\overset { \pi }{ = } O\\ \quad \quad \sigma \quad \quad \sigma \)
That's why H₂O molecule has bent structure whereas CO₂ molecule is linear.

H₂S-In the central atom is sulphur. There are 6 electrons in its valence shell (₁₆S = 2,8,6).Two electrons are shared with two H-atoms and the remaining four electrons are present as two one pair. Hence, total pairs of electrons are four(2 bond pairs and 2 lone pairs).
Due to the presence of 2 lone pairs the shape becomes distorted tetrahedral or angular or bent (non-linear).
PCl₃-In the central atom is phosphorus. There are 5 electrons in its valence shell (₁₆P = 2,8,5).Three electrons are shared with three Cl-atoms and the remaining two electrons are present as one long pair. Hence, total pairs of electrons are four(1 lone pairs and 3 bond pairs). Due to the presence of one lone pair, the shape becomes pyramidal (non-planar).